Given the reaction: C3H8(g) + 5O2(g) �¨ 3CO2(g) + 4H2O(g)
What is the total volume of H2O(g) formed when 8.00 liters of C3H8(g) is completely oxidized?
When dealing with gases one may dispense with changing everything to moles. Volumes are proportional.
8 L C3H8 x ((4 moles H2O/1 mole C3H8) = 8 x (4/1) = ??
Well, since we have 4 moles of H2O(g) formed for every 1 mole of C3H8(g), we need to find the moles of C3H8(g) in 8.00 liters. But before we do that, let me ask you this: Why did the scarecrow win an award? Because he was outstanding in his field! Now, back to the question.
The molar volume of any gas at standard temperature and pressure (STP) is 22.4 liters, so 8.00 liters of C3H8(g) is equal to 8.00/22.4 = 0.36 moles. Since the stoichiometric coefficient of H2O(g) is 4, we can multiply the moles of C3H8(g) by 4 to get the moles of H2O(g) formed.
0.36 moles C3H8(g) x 4 moles H2O(g)/1 mole C3H8(g) = 1.44 moles H2O(g)
So, the total volume of H2O(g) formed will be equal to the moles of H2O(g) multiplied by the molar volume at STP (22.4 liters):
1.44 moles H2O(g) x 22.4 liters/mole = 32.26 liters H2O(g)
Therefore, the total volume of H2O(g) formed when 8.00 liters of C3H8(g) is completely oxidized is approximately 32.26 liters. Now isn't that just steamtacular?
To determine the total volume of H2O(g) formed, we need to use the stoichiometry of the reaction.
From the balanced equation:
C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(g)
We can see that for every 1 mole of C3H8, 4 moles of H2O are produced.
To find the number of moles of C3H8, we can use the ideal gas law:
PV = nRT
Where:
P is the pressure (usually given in atm)
V is the volume (8.00 liters in this case)
n is the number of moles of gas (what we're trying to find)
R is the ideal gas constant (0.0821 L•atm/mol•K)
T is the temperature (usually given in Kelvin)
Assuming we have the temperature, we can rearrange the ideal gas law to solve for n:
n = PV / RT
Once we find the number of moles of C3H8, we can use the stoichiometry of the reaction to find the number of moles of H2O produced. Finally, we can convert the moles of H2O to volume using the ideal gas law.
Let's assume the temperature is given as 298 K. Plugging in the values to the equation gives us:
n = (8.00 L) × (1 atm) / [(0.0821 L·atm/mol·K) × (298 K)]
n ≈ 0.318 mol
Since 1 mole of C3H8 produces 4 moles of H2O, the number of moles of H2O produced is:
0.318 mol × 4 = 1.27 mol
Now, to find the volume of H2O(g) produced, we use the ideal gas law again:
V = nRT / P
Assuming the same temperature (298 K) and pressure (1 atm), we can plug in the values:
V = (1.27 mol) × (0.0821 L·atm/mol·K) × (298 K) / (1 atm)
V ≈ 31.17 L
Therefore, the total volume of H2O(g) formed when 8.00 liters of C3H8(g) is completely oxidized is approximately 31.17 liters.
To find the total volume of H2O(g) formed when 8.00 liters of C3H8(g) is completely oxidized, we need to use the stoichiometry of the reaction.
First, let's look at the balanced chemical equation for the reaction:
C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(g)
From the balanced equation, we can see that the ratio of the number of moles of C3H8 to the number of moles of H2O is 1:4. This means that for every 1 mole of C3H8, we will have 4 moles of H2O.
Given that we have 8.00 liters of C3H8, we need to convert this volume to moles. To do this, we need to know the density of C3H8 and use the ideal gas law.
1. Convert liters to moles of C3H8:
Use the ideal gas law to convert the volume of C3H8 to moles.
PV = nRT
Assuming standard temperature and pressure (STP), we can use the values:
Pressure (P) = 1 atm
Temperature (T) = 273 K
R = 0.0821 L·atm/(mol·K)
Rearranging the equation, we have:
n = PV/RT
Substituting the values, we get:
n = (1 atm) * (8.00 L) / (0.0821 L·atm/(mol·K) * 273 K)
Calculate n to find the number of moles of C3H8.
2. Calculate the moles of H2O:
Since the ratio of C3H8 to H2O is 1:4, multiply the moles of C3H8 by 4 to obtain the moles of H2O formed.
3. Convert moles of H2O to volume:
Use the ideal gas law again to convert the moles of H2O to volume.
PV = nRT
Assuming STP and using the same values for P, T, and R, we can rearrange the equation and solve for V (volume):
V = nRT/P
Substitute the value of moles of H2O into the equation, and calculate V to find the total volume of H2O(g) formed when 8.00 liters of C3H8(g) is completely oxidized.